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THE S-BLOCK ELEMENTS 299 THE s-BLOCK ELEMENTS 299 UNIT 10 THE s-BLOCK ELEMENTS The first element of alkali and alkaline earth metals differs in many respects from the other members of the group After studying this unit, you will be able to The s-block elements of the Periodic Table are those in ••• describe the general charact- which the last electron enters the outermost s-orbital. As eristics of the alkali metals and the s-orbital can accommodate only two electrons, two their compounds; groups (1 & 2) belong to the s-block of the Periodic Table. ••• explain the general characteristics Group 1 of the Periodic Table consists of the elements: of the alkaline earth metals and lithium, sodium, potassium, rubidium, caesium and their compounds; francium. They are collectively known as the alkali metals. ••• describe the manufacture, These are so called because they form hydroxides on properties and uses of industrially reaction with water which are strongly alkaline in nature. important sodium and calcium The elements of Group 2 include beryllium, magnesium, compounds including Portland calcium, strontium, barium and radium. These elements cement; with the exception of beryllium are commonly known as ••• appreciate the biological the alkaline earth metals. These are so called because their significance of sodium, oxides and hydroxides are alkaline in nature and these potassium, magnesium and metal oxides are found in the earth’s crust*. calcium. Among the alkali metals sodium and potassium are abundant and lithium, rubidium and caesium have much lower abundances (Table 10.1). Francium is highly radioactive; its longest-lived isotope 223Fr has a half-life of only 21 minutes. Of the alkaline earth metals calcium and magnesium rank fifth and sixth in abundance respectively in the earth’s crust. Strontium and barium have much lower abundances. Beryllium is rare and radium is the rarest of all comprising only 10–10 per cent of igneous rocks† (Table 10.2, page 299). The general electronic configuration of s-block elements is [noble gas]ns1 for alkali metals and [noble gas] ns2 for alkaline earth metals. * The thin, rocky outer layer of the Earth is crust. † A type of rock formed from magma (molten rock) that has cooled and hardened. 2019-20 300 CHEMISTRY Lithium and beryllium, the first elements increase in atomic number, the atom becomes of Group 1 and Group 2 respectively exhibit larger. The monovalent ions (M+) are smaller some properties which are different from those than the parent atom. The atomic and ionic of the other members of the respective group. radii of alkali metals increase on moving down In these anomalous properties they resemble the group i.e., they increase in size while going the second element of the following group. from Li to Cs. Thus, lithium shows similarities to magnesium 10.1.3 Ionization Enthalpy and beryllium to aluminium in many of their The ionization enthalpies of the alkali metals properties. This type of diagonal similarity is are considerably low and decrease down the commonly referred to as diagonal relationship group from Li to Cs. This is because the effect in the periodic table. The diagonal relationship of increasing size outweighs the increasing is due to the similarity in ionic sizes and /or nuclear charge, and the outermost electron is charge/radius ratio of the elements. very well screened from the nuclear charge. Monovalent sodium and potassium ions and divalent magnesium and calcium ions are 10.1.4 Hydration Enthalpy found in large proportions in biological fluids. The hydration enthalpies of alkali metal ions These ions perform important biological decrease with increase in ionic sizes. functions such as maintenance of ion balance Li+> Na+ > K+ > Rb+ > Cs+ and nerve impulse conduction. Li+ has maximum degree of hydration and 10.1 GROUP 1 ELEMENTS: ALKALI for this reason lithium salts are mostly METALS hydrated, e.g., LiCl· 2H2O The alkali metals show regular trends in their 10.1.5 Physical Properties physical and chemical properties with the All the alkali metals are silvery white, soft and increasing atomic number. The atomic, light metals. Because of the large size, these physical and chemical properties of alkali elements have low density which increases down metals are discussed below. the group from Li to Cs. However, potassium is 10.1.1 Electronic Configuration lighter than sodium. The melting and boiling All the alkali metals have one valence electron, points of the alkali metals are low indicating ns1 (Table 10.1) outside the noble gas core. weak metallic bonding due to the presence of The loosely held s-electron in the outermost only a single valence electron in them. The alkali valence shell of these elements makes them the metals and their salts impart characteristic most electropositive metals. They readily lose colour to an oxidizing flame. This is because the electron to give monovalent M+ ions. Hence they heat from the flame excites the outermost orbital are never found in free state in nature. electron to a higher energy level. When the excited electron comes back to the ground state, there Element Symbol Electronic configuration is emission of radiation in the visible region of the spectrum as given below: Lithium Li 1s22s1 Metal Li Na K Rb Cs Sodium Na 1s22s22p63s1 Potassium K 1s22s22p63s23p64s1 Colour Crimson Yellow Violet Red Blue Rubidium Rb 1s22s22p63s23p63d104s24p65s1 red violet Caesium Cs 1s22s22p63s23p63d104s2 λ/nm 670.8 589.2 766.5 780.0 455.5 4p64d105s25p66s1 or [Xe] 6s1 Alkali metals can therefore, be detected by Francium Fr [Rn]7s1 the respective flame tests and can be determined by flame photometry or atomic 10.1.2 Atomic and Ionic Radii absorption spectroscopy. These elements when The alkali metal atoms have the largest sizes irradiated with light, the light energy absorbed in a particular period of the periodic table. With may be sufficient to make an atom lose electron. 2019-20 THE s-BLOCK ELEMENTS 301 Table 10.1 Atomic and Physical Properties of the Alkali Metals Property Lithium Sodium Potassium Rubidium Caesium Francium Li Na K Rb Cs Fr Atomic number 3 11 19 37 55 87 Atomic mass (g mol–1) 6.94 22.99 39.10 85.47 132.91 (223) Electronic [He] 2s1 [Ne] 3s1 [Ar] 4s1 [Kr] 5s1 [Xe] 6s1 [Rn] 7s1 configuration Ionization 520 496 419 403 376 ~375 enthalpy / kJ mol–1 Hydration –506 –406 –330 –310 –276 – enthalpy/kJ mol–1 Metallic 152 186 227 248 265 – radius / pm Ionic radius 76 102 138 152 167 (180) M+ / pm m.p. / K 454 371 336 312 302 – b.p / K 1615 1156 1032 961 944 – Density / g cm–3 0.53 0.97 0.86 1.53 1.90 – Standard potentials –3.04 –2.714 –2.925 –2.930 –2.927 – E/ V for (M+ / M) Occurrence in 18* 2.27** 1.84** 78-12* 2-6* ~ 10–18 * lithosphere† *ppm (part per million), ** percentage by weight; † Lithosphere: The Earth’s outer layer: its crust and part of the upper mantle This property makes caesium and potassium 2 Na+→ O2 Na 22 O (peroxide) useful as electrodes in photoelectric cells. M+→ O2 MO2 (superoxide) 10.1.6 Chemical Properties (M = K, Rb, Cs) The alkali metals are highly reactive due to In all these oxides the oxidation state of the their large size and low ionization enthalpy. The alkali metal is +1. Lithium shows exceptional reactivity of these metals increases down the behaviour in reacting directly with nitrogen of group. air to form the nitride, Li3N as well. Because of (i) Reactivity towards air: The alkali metals their high reactivity towards air and water, tarnish in dry air due to the formation of alkali metals are normally kept in kerosene oil. their oxides which in turn react with moisture to form hydroxides. They burn Problem 10.1 vigorously in oxygen forming oxides. What is the oxidation state of K in KO ? Lithium forms monoxide, sodium forms 2 peroxide, the other metals form Solution – superoxides. The superoxide O2 ion is The superoxide species is represented as – stable only in the presence of large cations O2; since the compound is neutral, such as K, Rb, Cs. therefore, the oxidation state of potassium is +1. 4 Li+→ O2 2 Li2 O (oxide) 2019-20 302 CHEMISTRY (ii) Reactivity towards water: The alkali the highest hydration enthalpy which metals react with water to form hydroxide accounts for its high negative E value and and dihydrogen. its high reducing power. + − 2M+ 2H2 O →+ 2M 2OH + H2 (M = an alkali metal) Problem 10.2 – – It may be noted that although lithium has The E for Cl2/Cl is +1.36, for I2/I is + + most negative E value (Table 10.1), its + 0.53, for Ag /Ag is +0.79, Na /Na is reaction with water is less vigorous than –2.71 and for Li+ /Li is – 3.04. Arrange that of sodium which has the least negative the following ionic species in decreasing E value among the alkali metals. This order of reducing strength: behaviour of lithium is attributed to its – – I , Ag, Cl , Li, Na small size and very high hydration energy. Other metals of the group react explosively Solution with water. The order is Li > Na > I– > Ag > Cl– They also react with proton donors such as alcohol, gaseous ammonia and alkynes. (vi) Solutions in liquid ammonia: The alkali (iii) Reactivity towards dihydrogen: The metals dissolve in liquid ammonia giving alkali metals react with dihydrogen at deep blue solutions which are conducting about 673K (lithium at 1073K) to form in nature. + − hydrides. All the alkali metal hydrides are M++ (x y)NH3 → [M(NH3x ) ]+ [e(NH3y ) ] ionic solids with high melting points.
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